What is actual yield?

The amount of product actually produced during an experiment

the amount of product actually produced during repeated trials

the experimental value that you calculate

What is the formula for percent yield?

actual yield/ theoretical yield times 100

a reactant minus other reactant

experimental - actual/ actual times 100

theoretical yield/actual yield times 100

Balance this equation: C 4 H 10 + O 2 -> CO 2 + H 2

2C 4 H 10 + 13O 2 -> 8CO 2 + 10H 2 O

C 4 H 10 + 14O 2 -> 8CO2 + 10HO

9C 4 H 10 + 14O 2 -> 8CO2 + 10H 2 O

90CH10 + 14O 2 -> 8CO 2 + 10H 2 O

What is the excess reactant?

Th reactant that still has some left over and un used

the mass of the highest reactant

Determine the empirical and molecular formula of a compound that contains 45.71% C, 10.48% H, 30.48% O, 13.3% N. It's molar mass is 210 g/mol.

emp: C 4 H 11 O 2 N mol: C 8 H 22 O 4 N

emp:C 3 H 8 O 2 N mol: C 6 H 16 N2

emp: C 4 H 10 ON mol: C 12 H 3 OO 3 N 3

In the __________ reaction following: 2 C 8 H18 + 25 O 2 > 16 CO 2 + 18 H 2 O, how many moles of oxygen gas are required for the complete ___________of 56.0 moles of Isooctane (C 8 H 18 )?

combustion ; 711.25 mol C 8 H 18 ; combustion

combustion; 6.25 mol of C 8 H 18 ; combustion

double replacement; 710.34 mol C 8 H 18 ; double replacement

synthesis; 53.26 mol C 8 H 18 ; synthesis

Stoichiometry Chemistry Quiz;

Science, Chemistry

9th Grade

NGSS covered

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25 questions

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MULTIPLE CHOICE QUESTION

1 min • 1 pt

Convert 1.25 mol Ca into atoms Ca

6.25 atoms Ca

7.53 x 10²³ atoms Ca

8.38 x 10²⁴ atoms Ca

1.23 x 10²³ atoms Ca

MULTIPLE CHOICE QUESTION

45 sec • 1 pt

Write the equation for percent by mass of an element in a compound?

mass of element in the compound / molar mass of the compound * 100

molar mass of the compound / mass of element in the compound molar mass of the compound * 100

molar mass = mass of element in the compound / mass of the pressure

mass of pressure over 10

Tags

NGSS.HS-PS1-7

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

The empirical formula is the formula of a compound in which the subscripts are reduced to the-

Highest

Lowest

Most

Medium

MULTIPLE CHOICE QUESTION

1 min • 1 pt

What is the molecular formula?

is reduced

It is the formula in which the subscripts specify the actual number of atoms of each element in one molecule or formula unit of the substance.

is in the simplest form

is in the highest form that it can be

Tags

NGSS.HS-PS1-7

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

Trichlorobenzen has an empirical formula of C2HCL and a molar mass (molecular formula mass) of 181.44 g/mol. What is the molecular formula of trichlorohenzene?

C₆H₃Cl₃

C₂ClH

C₄H₂Cl₃

C₈H₄Cl₅

Tags

NGSS.HS-PS1-7

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

A compound is 54.5% carbon, 9.1% hydrogen, and 36.4%
oxygen by mass. Its molar mass is 88.1 g/mol. What is its empirical and molecular formula?

H₃C₄O₉, C₂HO₂

C₅H₂O₄, H₂C₈O₃

C₂H₄O₂, C₄H₈O₂

C₄H₈O₂, C₂H₄O₂

Tags

NGSS.HS-PS1-7

NGSS.HS-PS1-2

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What would this reaction be : 1MgF₂ + 1Li₂CO₃ -> 1MgCO₃ + 2LiF

Double Replacement

Single Replacement

Synthesis

Neutralization

Tags

NGSS.HS-PS1-2

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Stoichiometry Chemistry Quiz;

Convert 1.25 mol Ca into atoms Ca

Write the equation for percent by mass of an element in a compound?

The empirical formula is the formula of a compound in which the subscripts are reduced to the-

What is the molecular formula?

Trichlorobenzen has an empirical formula of C2HCL and a molar mass (molecular formula mass) of 181.44 g/mol. What is the molecular formula of trichlorohenzene?

A compound is 54.5% carbon, 9.1% hydrogen, and 36.4%
oxygen by mass. Its molar mass is 88.1 g/mol. What is its empirical and molecular formula?

What would this reaction be : 1MgF₂ + 1Li₂CO₃ -> 1MgCO₃ + 2LiF

How many moles of Potassium bromide are formed when 0.236 moles of Aluminum sulfate are also formed? 2AlBr₃ + 3K₂SO₄ -> 6KBr + 1Al₂(SO₄)₃

What is the mass of Beryllium fluoride when it is required to produce 122.5 grams of Rubidium fluoride? 2RbNO₃ + 1BeF₂ -> 1Be(NO₃)₂ + 2RbF

What is the theoretical yield (grams) of silver produced from 6.2 moles of copper and an excess of silver nitrate? 2AgNO₃+ 1Cu -> 1Cu(NO₃)₂+ 2Ag

Access all questions and much more by creating a free account

Popular Resources on Wayground

Discover more resources for Science

Stoichiometry Chemistry Quiz;

Convert 1.25 mol Ca into atoms Ca

Write the equation for percent by mass of an element in a compound?

The empirical formula is the formula of a compound in which the subscripts are reduced to the-

What is the molecular formula?

Trichlorobenzen has an empirical formula of C2HCL and a molar mass (molecular formula mass) of 181.44 g/mol. What is the molecular formula of trichlorohenzene?

A compound is 54.5% carbon, 9.1% hydrogen, and 36.4% oxygen by mass. Its molar mass is 88.1 g/mol. What is its empirical and molecular formula?

What would this reaction be : 1MgF2 + 1Li2CO3 -> 1MgCO3 + 2LiF

How many moles of Potassium bromide are formed when 0.236 moles of Aluminum sulfate are also formed? 2AlBr3 + 3K2SO4 -> 6KBr + 1Al2(SO4)3

What is the mass of Beryllium fluoride when it is required to produce 122.5 grams of Rubidium fluoride? 2RbNO3 + 1BeF2 -> 1Be(NO3)2 + 2RbF

What is the theoretical yield (grams) of silver produced from 6.2 moles of copper and an excess of silver nitrate? 2AgNO3 + 1Cu -> 1Cu(NO3)2 + 2Ag

Access all questions and much more by creating a free account

Popular Resources on Wayground

Discover more resources for Science

A compound is 54.5% carbon, 9.1% hydrogen, and 36.4%
oxygen by mass. Its molar mass is 88.1 g/mol. What is its empirical and molecular formula?

What would this reaction be : 1MgF₂ + 1Li₂CO₃ -> 1MgCO₃ + 2LiF

How many moles of Potassium bromide are formed when 0.236 moles of Aluminum sulfate are also formed? 2AlBr₃ + 3K₂SO₄ -> 6KBr + 1Al₂(SO₄)₃

What is the mass of Beryllium fluoride when it is required to produce 122.5 grams of Rubidium fluoride? 2RbNO₃ + 1BeF₂ -> 1Be(NO₃)₂ + 2RbF

What is the theoretical yield (grams) of silver produced from 6.2 moles of copper and an excess of silver nitrate? 2AgNO₃+ 1Cu -> 1Cu(NO₃)₂+ 2Ag